1. 15.8 g of KCl is dissolved in 225 mL of water. Calculate the molarity. 2. Calculate the mass of KCl required to prepare 250. mL of 0.250 M solution.
BE READY WITH THE STOPWATCH. Record the time in the data table. Room Temperature Water: Fill beaker with 80mL of water. Use thermometer to record the temperature Drop Alka-Seltzer tablet in water. Measure the time it takes to completely dissolve.
After that, dissolve the sample in 2 mL of deionized water and shake the test tube for 1 to 1 ½ minutes to dissolve the solid. Place another dry test tube in a 50mL beaker and weigh it. Find a bottle of barium iodide and record the name and molar mass. Then, weight out either anhydrous barium iodide or barium iodide dehydrate into this test tube and dissolve is it in 2 mL of deionized water. Pour the contents of one of the test tubes into the other and a reaction should occur and you should see a white precipitate of barium sulfate form.
Part C: Density of an Irregular Shaped Solid 1) Obtain a sample of metal and determine the mass. 2) Fill a 100 mL or 50 mL graduated cylinder with water, recording its volume. 3) Using the water displacement method, determine the volume of the object. 4) Determine the density and percent error. Part D: Density of Methanol 1) Find the mass of an empty 10 mL graduated cylinder, and then fill approximately 9 mL of methanol and record volume.
Hydrate Lab The purpose of this lab is to analyze the percent water in a crystalline hydrate and to indentify the hydrate from a list of possible unknowns. The solid hydrate will be heated to remove the water, and the percent can be found by measuring the mass of the solid before and after heating. The hydrate will be indentified by comparing the percent water in the hydrate with the percent water calculated for the possible unknown. Before the lab there are pre-lab questions: 1. Describe the three general safety rules for working with a Bunsen burner.
-Name of the experiment: The study of titration (volumetric analysis) -Purpose: To investigate the titration two standard solutions with opposite pH values and the relationship between pH value and volumes of the reactants. Use this method to determine active ingredients in a commercial basic product. -Task Procedure: Section 1: The making of a standard solution of sodium hydroxide. Section 2: The use of a pH probe and computer program to produce a simple titration curve. Section 3: The titration of an unknown concentration of HCl with the standard solution of NaOH.
3. Take off the hot plate when the bubbling of the crystals has stopped. 4. Let cool and mass the evaporating dish and alum. 5.
The aspirator was turned to medium high, and then the copper was poured onto wetted filter paper. Using distilled water to remove all copper from the beaker. Once completely on filter paper 6mL of acetone was added to the copper to help dry it out. The filter paper was then removed and set down to dry completely. Once dry the filter paper was weighed with the copper on it and subtracted from the original weight to see the amount of copper left after
Obtain another 50-mL beaker and add 0.05g of Chromium(III) Nitrate to the beaker. Then, add 17 mL of distilled water and mix until the solid is dissolved. 3. Obtain a final 50-mL beaker and add 0.05 grams of the unknown substance to the beaker. Add 17 mL of distilled water and mix with a stir bar until the solid is completely dissolved.
This solution was placed in a burette and 18.4 cm3 was required to neutralise 25 cm3 of 0.1 moldm-3 NaOH. Deduce the molecular formula of the acid and hence the value of n. 5. Sodium carbonate exists in hydrated form, Na2CO3.xH2O, in the solid state. 3.5 g of a sodium carbonate sample was dissolved in water and the volume made up to 250 cm3. 25.0 cm3 of this solution was titrated against 0.1 moldm-3 HCl and 24.5 cm3 of the acid were required.